Jan Robert Selman UCRL-20 557 o.Q
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MEASUREMENT AND INTERPRETATION OF LIMITING CURRENTS
Jan Robert Selman (PhD, Thesis) June 1971
AEC Contract No0 W-7405-eng-48
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\ LAWRENCE RADIATION LABORATORY U-' IF U UNIVERSITY of CALIFORNIA BERKELEY DISCLAIMER
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Table of Contents Abstract . Introduction
Chapter 1. Applicability of the limiting current method Part The limiting current method
I.I. The limiting current ...... 3 1.2. Measurement of mass transfer rates ...... 5 1.3. Model reactions ...... 7 * 1.4. Historical ...... 11 Part Review-of applications 1.5. Simple laminar flows ...... 14 1.6. Laminar flow with complications ...... 25 1.7. Turbulent flows and mixed convcctjcrt ...... 40 1.8; Restricted cells with agitation ...... 52 1.9. Cells with gas-evolution ...... 55 1.10. Particulate flow systems ...... 58 1.11. Electrochemiluminescence ...... 61 1.12 Conclusions ...... 61 Chapter 2. Validity of the limiting current method
Part Basic concepts of electrochernical mass transfer 2.1. Migration and diffusion ...... 67 2.2. Polarization ...... 77 2.3. Current and potential distribution ...... 91 Part Conditions for validity 2.4. Definition of the ii nitin, current pIteau 105 2.5. Conç1ition' ror valid mcxcu1epnt 105 2.6. (oditiç for valjc1 1ntcF1ctat1on 10u -11-
Chapter 3. Rotating disk integral diffusivities of Cu ion in CuSO4 - H2SO4 -H20
3 .1.. Introduction ...... 108
3 .2. Experimental ...... 110
3.3. Results • ...... 118
3.4. Discussion: migration effect ...... 138
3.5. Discussion: deposit roughness ...... 147 3.6. Conclusions ...... 157
Chapter 4. Unsteady state effects in electrochemical flow cells Part I. Review
4.1. Introduction ...... 161
4 .2. Free conyection . ...... 162
4 .3. Forced convection ...... 169 4.4. Interaction with potential. distribution at
elongated electrodes . • ...... 172 Part II. Unsteady state at a rotating disk electrode -
4 .5. Experimental ...... 177
4 .6. Results ...... 179
4 .7. Discussion ...... 194
4.8. Conclusions ...... 208
Conclusions and Recommendations ...... 210
Acknowledgments ...... 2]3
• Appendices . . • •
• A. Program for calculation of a theoretical limiting
currcnt curve -. . ...... ... . 214 -ill-
Flux at a rotating disk electrode after a concentration
step at the surface, in the limitof high Schmidt numbers . . 216
Degree of dissociation of HS0 ion in the system CuSO 4
-H2SO4-H20 237 Migration at a rotating disk electrode in acidified solutions
of CuSO4 characterized by the bisulfate dissociation
parameter I/K = 5 ...... 250
Theoretical solutions for transient convective diffusion . . 256 Transient diffusion following linear potential decrease at a
redox electrode ...... 261 C. Transient diffusion following linear' potential decrease for
a deposition reaction, taking electrode kinetics
into account ...... 270
Nomenclature ...... 288
References...... 295 MEASUREMENT AND INTERPRETATION OF LIMITING CURRENTS
Jan Robert Selman
Inorganic Materials Research Division, Lawrence Radiation Laboratory Department of Chemical Engineering University of California, Berkeley, California
June 1971
ABSTRACT
Applications of the limiting current method for measuring mass transfer rates are reviewed. To date almost 100 publications using this method have appeared, with recent applications in the area of stirred tanks, parti- culate systems, mixed convection and turbulence.
The conditions for valid measurement and interpretation of limiting currents are discussed. An ideal limiting current curve is constructed for the copper deposition model reaction. The effect of migration due to the electric field is computed for this reaction, taking into account that the bisulfate ion is not completely dissociated. The use of integral dif - fusivities, which reflect the effect of migration as well as that of variable physical properties, is required in the correlation of mass transfer coefficients calculated from limiting currents.
Rotating disk integral diffusivities are reported for cupric ion in acidified solutions of cupric sulfate In solutions containing less than 0.1 molar cupric sulfate the product of viscosity and integral diffusivity is independent of the ionic strength of the solution. In more concentrated solutions the effect of surface roughness developing near the limiting current is discernible in high dffusivitv values. Some semi-quantitative
COflSlderdtlons on the developncnt-ard extent of this ioughness effect are given -vi -
Unsteady-state effects in limiting current measurements are reviewed from the viewpoint of nonstationary convective diffusion. The complicating effect of the presence of an electric field is discussed, and it is shown that apparent, nonsimultaneous, sectional limiting currents can be expected to occur at elongated electrodes. Unsteady-state limiting currents at a rotating disk electrode are investigated experimentally, using the fern- cyartide-ferrocyanide redox system. The minimum time to reach a steady-state limiting current by linear current increase is an order of magnitude larger than that necessary if a linear potential scan is applied. Apparent limiting currents due to fast current increase or potential scan rates can be satis- factorily interpreted in terms of a pure-diffusion model.
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INTRODUCTION : STRUCTURE OF THE THESIS
Electrochemical measurements of mass transfer rates by the limiting
current technique have been employed in recent decades with increasing
frequency. The present work aims to contribute to the methodology of limit-
ing current measurements by a unifying review of applications and of con-
ditions for validity, as well as by a detailed study of some critically important aspects.
In the first Chapter the basic features of the method are described,
its advantages and limitations.. The varIety of mass transfer situations
towhich it has been applied, is reviewed. . . .
Chapter 2 gives a synopsis of those concepts of electrochemical
mass transfer theory which are necessary 'for an analysis of the limiting
current'.conditjon. The requirements for an. effective meaurement and a
valid interpretation of the results, are reviewed.
Three practical aspects of the limiting current technique are singled out for a detailed investigation: diffusivity values appropriate
to the method, unsteady-state mass transfer during the approach of the
limiting current, and the effect of current distribution below and at
the limiting current, due to the presence of an electric field.
Chapter 3 treats the problem of appropriate diffusivities to be used in limiting current studies, in particular for the copper deposition
reaction frequently used in free-convection studies It is shown that migration and surface roughness formed near the limiting current both have a considerable effect on the integral diffusivities measured at a rotating disk electrode The conditions under which the surface roughnes'- effect is minimal are investigated.
Chapter 4 deals with the unsteady state due to mass transfer.
Available information concerning transients in convective diffusion is
• reviewed. From a comparison with experimental limiting current curves
at planar, sectioned electrodes it can be inferred that transient ef-
fects are more persistent than expected. This is shown to be related
to the current distribution below the limiting current. • • • The second part of Chapter 4 is devoted to astudyof unsteady-
state mass transfer at a rotating disk electrode, using a redox reaction where such current distribution effects are not important. The apparent
limiting currents observed, in fast current ramps or potential scans are • . explained in terms of a pure-diffusion model. •
/ • • • 3
Chapter 1 APPLICABILITY OF THE LIMITING CURRENT METHOD Part 1. The limiting current method
1.1. The limiting current.
• The term "limiting current density" is used to describe the maximum rate at which a particular electrode reaction can proceed in the steady state, with 100% current efficiency. This rate is determined by the composition and transport properties of the electrolytic solution on the one hand, and on the other by the hydrodynamics of the electrochemical cell In a given situation the limiting current at an electrode can only be exceeded by increasing the cell pOtential until another consecutive, electrode reaction starts occurring at finite rate
The limiting current may be due to a slow,rate-determining step in the electrode reaction (kinetic limiting current). However, in the majority of cases where a limiting current is encountered it is caused by the slowness of transport of ionic or uncharged species through the solution The ions (or molecules) move toward the electrode where they are consumed in the electrode reaction, or a reaction coupled with it
Electrode reactions, by their nature, are surface reactions and cause local changes in composition A thin diffusion layer, impoverished in the reacting species, develops at the electrode surfaces The ions or mole- cules move across the diffusion layer by diffusion down concentration gradients. Ions move also under the influence of the electric field, i e , they migrate
Limiting currents are usually associated with cathodic reactions (e g in metal deposition), although anodic reactions are by no means excluded
Whenever the supply of a dissolved species from the solution to the elec- trode surface becomes a rate limiting factor, limiting Lurrent phenomena 4
may be observed. Agar.and Bowden 122 showed that diffusion of H20 limits
0 2 evolution in fused NaOH. Hoar and Rothwell 28 observed anodic limiting currents in electropolishing of copper, due in part to a dissolution
diffusion layer, and in part to a solid oxide film.
In most cases the diffusion layer is not a stagnant layer, as
presented in the early Nernst-Whitman model. Where no forced convection
is maintained free convection usually sets in due to the density gradient
developing in the diffusion layer. The convective velocity, although it
vanishes at the wall, enhances the diffusion toward the electrode. It
steepens the concentration gradient of the reacting species at the elec-
trode and therefore increases the maximum current obtainable.
Equivalently this is often expressed as a decrease of the Nernst
layer thickness. In the stagnant layer model referred to above the con-
centration profile of the reacting ion is linear, with the thickness
chosen so as to give the actual concentration gradient at the electrode.
This fictitious 6 is always smaller than the real diffusion layer thick- ness, but better defined since the actual concentration profile tapers off very gradually to the bulk value.
clearly the maximum gradient for a certain rate of stirring, i.e., a given hydrodynamic condition near the electrode, is that gradient where- by the concentration at the electrode is reduced to zero, or virtually zero. This situation corresponds, in an electrochemical cell, to the limiting current condition. S
1 2 Measurement of mass transfer rates
If the rate ofthe reaction is not restricted by the kinetics of
the reaction mechanism, the reaction is called "reversible and its
rate is transport-controlled The current density, i, is proportional to
the reacting ion (or molecule) flux, N., byFaraday's law:
s.i = -nFN. (1.1) 1 - -1
Here.s is the number of molecules of speciesi participating in the
transfer of n electrons to or from the electrode.
Therefore, if the driving force of the mass transfer process can be expressed in a practical form, e.g., as a concentration gradient of the reacting species, or as a concentration difference betw.een electrode and bulk solution, one can relate the mass transfer rate in a general way to the concentration driving force. If the concentration gradient is known, an effective diffusivity can be defined
N = _Deff Vc (1.2)
More often, only the concentration difference electrode/bulk is known, and in such cases the mass-transfer coefficient can be calculated:
N = k(clO_clb) (1.3)
In the limiting current method of measuring mass transfer coefficients, the reacting ion concentration at the electrode is made vanishingly small by applying a large potential In that case only the current density and the bulk concentration need to be known 6
If the concentration at the electrode is not zero, it can still be measured by optical techniques, in particular by interferometric methods.
Such measurements, however, are relatively simple only in dilute solu 115 tions, because refraction occurs in addition to interference. More- over, they are restricted to solutions where only the reacting species concentration varies, i e , to solutions of a single salt If the solu- tion contains two electrolytes with dissimilar concentration profiles in the diffusion layer, a second, independent, measurement is needed to establish the reactant concentration at the electrode.
In practice such multicomponent electrolytic solutions are used much more frequentlythan those of singlesalts. In binary solutions the current exceeds the expected current due to. convective diffusion by a factor of approximately two. This excess current is due to migration of the reacting . ion in the electric field. It can be suppres,sedby increasing the conductivity of the solution, thereby lowering the elec- tric field strength. Thus, in mass transfer measurements, a large amount of "supporting" or "inert" electrolyte is usually added to the solution.
The complications associated with the presence of non-reacting ions in the diffusion layer have been discussed extensively elsewhere1131114
They. are of special importance in free convection, where the driving force, i.e., a density difference, is affected by the accumulation or deficit of non-reacting ions at the electrode. In both forced and free convection it is important to know the ion flux contributed by migration, which is never completely absent. Chapter 2 deals with this problem in quantitative terms. 7
Since current measurements can be made very exactly, the limiting
current technique is a convenient and precise method of measuring mass
transfer rates. The limiting current makes itself knownas a plateau
or inflection point in the plot of current versus electrode overpotential
(Figure 3.6). In principle the accuracy of mass transfermeasurements is
limited only by the precision with which this limiting current plateau,
or point, can be read. Further, the electrode area, current distribution
and reactant bulk concentration have to be known accurately.
1.3. Model reactions.
The electrochemjcal reactions most often used for the study of
limiting currents are listed in Table 1.1. Oxygen reduction was used • 87 . in early experiments with a rotating disk. Later many investigators made use of copper deposition from acidified solution. This reaction
has the disadvantage of changing the cathode surface, especially near
the limiting current where the deposit becomes rough (see section 3 5 )
For forced convection studies copper deposition has been largely
supplanted by the reduction of ferricyanide at a nickel or platinum
surface. Usually, an equimolar mixture of fern- and ferrocyanide is
used. The oxidation of ferrocyanide at the anode compensates, at least
in part, for the cathodic depletion of ferricyanide, if anolyte and catholyte are not separated by a diaphragm The ferrocyanide oxidation reaction has also been used occasionally as the controlling reaction, but it has the disadvantage of a shorter limiting current plateau In addition, oxygen evolution passivates a nickel anode (Both electrodes 8
Table Li. Model reactions in electrochemical mass transfer studies. Ilk
E°(v) electrode supporting reference
metal electrolyte -
CAThODIC many 1 Fe(CN) + e -* Fe(CN) +0 360 Ni,Pt 6 6
NaOH 2,87 2 02 + 2H20 + 4e - 40H +0 401 Pt,Ag
3 1 3 + 2e -* 31 +0 536 Pt KI 59,88
fosfate 4 +2H + 2e - +0 699 Ag 2 0 OOH buffer
s z2n + 2e Zn -0 763 Zn(Hg) KOH
6 Cd 2 + 2e - Cd -0 352 Cd(Hg) none 4 2+ H SO many 7 Cu + 2e Cu +0. 337 Cu 2 4 none 7,9,23
8 Ag + e - Ag +0 799 Ag HC10 4 5
ANODIC
9 CuCl -* CuCl + e +0 153 Pt CaCl 15 4 4 2 many 10 Fe(CN) -* Fe(CN) + e +0 360 Ni,Pt
4 9
are susceptible to CN poisoning. The correct procedure to activate
nickel electrodes before use has been described by Eisènberg c.s. 6 )
For studies of free convection mass transfer, or combinations of
forced and free convection, the copper deposition reaction remains the
preferred reaction, in spite of the precautions necessary to prevent
excessive surface roughening near the limiting current The advantage that copper deposition offers in such studies is a considerably larger driving density difference, due to (1) its higher solubi.lity; (2) the
larger densification (see Table 1.2).
In the case of the redox reaction the opposite effects of reactant depletion and product accumulation canceleach other to a large extent.
The densification due to ferrocyanide is larger than that due to fern- cyanide (each larger than that for CuSO4 ), so that the redox reaction makes the catholyte denser and the anolyte less dense
The actual densification is also influenced by the effect of migration. As shown in the third line of Table 1.2, the relative densifi- cation in acidified cupric sulfate is less than in binary cupric sulfate solution. In the case of the supported redox reaction the migration effect makes the density difference larger than expected from over-all reaction stoichiometry.
None of the other reactions listed in Table 1.1 have attained the popularity of ferricyanide reduction and copperdeposition. The oxygen and iodine reduction reactions satisfy the requirements of a reasonably long plateau (> 250 my, depending on the supporting electrolyte pH) and do not change the surface They are however restricted to forced convec- tion situations with large flow rates, since the bulk concentrations are 10
Table 1.2. Maximum densification in cupric sulfate and alkaline equimolar fern-and ferrocyanide solutions, at 25 ° C.
CuSO4 CuSO4 equimolar ferri/ferrocyanide +2.OM NaOH
+l.5M HS02 4
cathodic anodic
LcR(M) 1.4 0.9 0.2 0.2 cLR(M1) 0.140 0 140 0.167 0 226 tsp/p 0.140 0 125 -0 0706 0.0832 p(g/ml) 1.214 1.217 1.50
(cp) 1.824 1.914 1.647 v(cst) 1.502 1.573 1.432
Ap(g/ml) 0.170 0.137 -0 0812 +0 0957
Values of aR and Ap/p taken from Ref. 114
1. 11
of the order of 10 3M at most. Reducible impurities and gases (e.g.
02 if iodine is the reactant) have to be rigorously excluded In the case of oxygen reduction, maintaining a known oxygen concentration in the bulk.is not a trivial problem because of the tendency to super- saturation, and the extreme sensitivity of the solubility to the salt concentration in solution.
The silver and zinc deposition reactions have only occasionally been used. Dendritic deposits form very easily unless organic inhibitants are added,. which complicates the electrode kinetics to the point of obscuring the limiting current
In the present study only ferricyanide reduction and copperdeposition were employed.
144. Histo±ica1.
The dependence of current density on the rate of stirring was first 116 117 clearly established by Nernst and Brunner (1904). They interpreted this by means of the stagnant layer concept first used by Noyes and Whitney.
The thickness of this layer ("Nernst diffusion layer thickness") was correlated simply with the speed of the stirring impeller or rotating electrode tip
The lack of hydrodynamic definition was recognized by Eucken, 99 who considered convective diffusion transverse to a parallel flow and obtained an expression analogous to the Lvque equation of heat transfer.
Experiments with Couette flow between a rotating cylinder and a station- ary outer cylinder did not confirm his predictions At very low rotation rates, where such a flow is stable, it does not contribute to the diffusion process since there is no velocity component in the radial 12
direction At higher rotation rates secondary flow patterns form (Taylor
vortices) and finally the flow becomes turbulent Neither flow regime satisfies the conuitions of the Lvque equation
However, flow generated by a cylinder rotating at high speed was 118 119 subsequently used by others, in particular King and co-workers ' to demonstrate that dissolution proLesses are diffusion limited, and electro-
chemical corrosion processes as well The dependence of the mass-transfer coefficient on the 0.7 power of rotation rate and diffusivity of the
dissolving species was established (cf. Table 1.3, eq. 31).
Of considerable importance for the conceptual development of limit-
ing current measurement was the work of Agar and Bowden 122 on the current- overpotential relationship at nickel electrodes in fused sodium hydroxyde, where water transport is the limiting step
2OH+-O2 +H2O+e
A more detailed review of this, and other, early work in ionic mass
transfer is given by Tobias, Wilke and Eisenberg 100
The full development of electrochemicai techniques of mass transfer
measurement had to await the formulation of a quantitative insight into
the role of convective diffusion in electrode processes. This was first
successfully provided by the groundbreaking work of Levich on the rotating
disk electrode,9 5 ' 106 so that by 1947 the conditions were fuli11ed for
a matching of theory and practice. 87 Agar 107 pointed out that electro- chemical mass transfer correlations should be closely similar to those known for heat transfer The first test of the theory of convective diffusion in free convection was made by Wagner. 1 From 1951 on limiting 13
current measurements have been used with increasing frequency and Lonfidence
to establish mass transfer •rates.at reactive surfaces in flow situations
where they cannot be predicted on theoretical grounds, or where the theory needs confirmation.
Only a few reviews have appeared in which the application of the
method is discussed from a chemical engineering viewpoint In the review
already mentioned Tobias, Wilke and Eisenberg 100 examined the available knowledge about electrochemical mass transport at the beginning of its
application (1950). The same authors developed correlations for predicting
the limiting current in laminar free convection at vertical electrodes, as well as in turbulent flow between cylindrical electrodes, with the inner cylinder rotating and the outer one stationary.
Ibl 8 reviewed early work on free convection, to which he and his co- workers contributed notably by the development of optical methods for the study of the diffusion layer. 101 ' 7 ' 9 A discussion of their application falls outside the scope of this review and has been given by Muller. 104 102 In a survey of 1963, Ibl lists 13 mass transfer correlations established by the limiting current method. Only 4 of these were known from quantitative theoretical predictions. The total number of publica- tions since 1963 has almost quadrupled (references 1-88) The majority of these concern flow situations where theoretical predictions are at most of a qualitative nature An increasing number of publications deal with model studies of complex situations, e g , packed and fluidized beds, and with hydrodynamic studies. 14
Part II. Review of Applications
For the purpose of this review we will distinguish experimental
studies of mass-transfer in: (a) simple laminar flow; (b) laminar flow with
complications; (c) turbulent flow and mixed convection; (d) stirred vessels; (e) cells with gas-evolution; (f) particulate flow systems.
A related technique of mass transfer measurement will also be discussed briefly.
1.4. Simple laminar flows
For the flow situations listed as number. 1 through 5 in Table 1.3 the mass transfer rate can be derived directly from a solution of the equa- tion of convective diffusion. The velocity profile near the electrode is known, and the equation is simplified by appropriate similarity transforma- tions. Newman 103 has reviewed these solutions in detail. Here we only want to comment on the nature of the velocity profile near the electrode, and on the agreement between theory and experiment
In the case of the rotating disk there is a uniform axial velocity towards the disk, which depends only on the normal distance from the disk, so that the mass transfer rate is also uniform. If the center of the disk is non-reactive, the flux to the active ring is higher than itotherwise would be, and the electrode is no longer uniformly accessible. The maximum rate is found at the inner edge of the ring, where radial convection is no longer uniform. Thus, the maximum is due to the non-coincidence of the uniform hydrodynamic boundary layer and the diffusion layer (relaxation process). 15
Table 1 3 Mass transfer correlations obtained by limiting current measure- .ments.